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Vladimir79 [104]
3 years ago
11

Which compound has the LEAST percent composition by mass of sulfur?

Chemistry
1 answer:
Eddi Din [679]3 years ago
5 0

Answer: srs with 32.38 grams

Explanation:

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Which pair of elements is MOST likely to chemically combine and form ionic bonds?
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The right answer for the question that is being asked and shown above is that: "C. carbon and hydrogen." The pair of elements is MOST likely to chemically combine and form ionic bonds are <span>carbon and hydrogen </span>
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The concentration of reactant doesn't affect the activity
pashok25 [27]

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B.false because if the reactant concentration is disturbed the whole reaction will be affected.

Explanation:

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How many moles of aluminum oxide (Al2O3) can be produced from 12.8 moles of oxygen gas (02)
zhannawk [14.2K]

Answer:

Theoretical Yield

Percent yield

Example stoichiometry problem

How much oxygen can be prepared from 12.25 g KClO3 . (Use molar mass KClO3 = 122.5 g.)

Most stoichiometry problems can be solved using the following steps.

Step 1.

Write and balance the equation for the decomposition of KClO3 with heat (∆). 2KClO3 + ∆ → 2KCl + 3O2

Step 2.

Convert what you have (in this case g KClO3) to moles.

# moles = grams/molar mass = 12.25 g /122.5 = 0.100 mole KClO3.

Step 3.

Using the coefficients in the balanced equation, convert moles of what you have (moles KClO3) to moles of what you want (in this case moles oxygen).

0.100 mol KClO3 x (3 moles O2/2 moles KClO3) = 0.100 x (3/2) = 0.150 mole O2.

Step 4.

Convert moles from step 3 to grams.

moles x molar mass = grams

0.150 mole O2 x (32.0 g O2/mole O2) = 4.80 g O2 produced from 12.25 g KClO3. This is the theoretical yield. If the ACTUAL yield is 4.20 grams, calculate percent yield. Percent yield = (actual yield/theoretical yield) x 100 = (4.20/4.80) x 100 = 87.5% yield

NOTE: In step 1, moles can be obtained other ways; in step 4 moles can be converted to other units.

a. For solutions, M x L = moles (or mL x M = millimoles).

b. For gases, L/22.4 = moles

4 0
3 years ago
How would you prepare 100 ml of 0.4 M MgSO4 from a stock solution of 2 M MgSO4?
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<span>M1V1 = M2V2 
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M1 = 2M
V1 is the unknown
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V2 = 100 ml

</span>plug in the givens in the above equation:
<span>2 x V1 = 0.4 x 100 
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V1 = 20 ml

Based on this: you should take 20 ml of the 2 M solution and make volume exactly 100 ml in a volumetric flask by diluting in water.

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Answer:

Foam fight is a chemical change.

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